Question 14Trial # Initial A (M) Initial B (M) Initial Rate (M/s)10.2000.2001.20 x 10-320.2000.4002.40 x 10-330.4000.2004.80 x 10-3Given the table above, use trial #3 to determine k.

To determine the rate constant kkk for trial #3 using the given table, we follow the same approach…

Answered: Question 14 Trial # Initial A (M)…

Chemistry

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Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question 1 For the hypothetical reaction A + 3B -->2C, the rate of appearance of C, given by ( A[C]/At, may also be expressed as A A[C]/At = - A[A]/At B A[C]/At = - (3/2) A[B]/At C A[CI/At = - (2/3) A[B]/At ΔΙΟ/Δt - -(1/2) ΔΙΑΙ/Δt O A O B O C O D
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A 100% 7:07 PM Wed Feb 5 Unanswered •1 attempt left For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 10.015 M 0.200 M 3.67 × 10^-6 20.030 M 0.200 M 7.33 × 10^-6 3 0.015 M 0.400 M 1.47 × 10^-5 The special rate constant k 1.2 x 10^-3 (1/M•sec) 9.2 × 10^-4 (1/M•sec) 1.6 x 10^-3 (1/M-sec) 6.1 × 10^-3 (1/M^2·sec) D 8.2 x 10^-3 (1/M^2•sec) Submit ш
What is the reaction constant and the rate law of the reaction in the table?
Examine the experimental data shown in the table below for the following reaction: A + 5B + 6C ---> 3D + 3E Experiment [A] (M) [B] (M) [C] (M) Rate (M/s) 1 0.35 0.35 0.35 8.0 x 10-4 2 0.70 0.35 0.35 3.2 x 10-3 3 0.70 0.70 0.35 6.4 x 10-3 4 0.70 0.35 0.70 3.2 x 10-3 A) what is the reaction order of A? B) what is the reaction order of B? C) what is the overall rate equation for this reaction? D) what is the value of the rate constant? E) what are the units of the rate constant?
Using the following chemical equation and data: 3A + B + 2C --> D + 2E Experiment Initial [A] Initial [B] Initial [C] Initial Rate 1 1.0 x 10-2 4.0 x 10-3 2.0 x 10-2 5 mM/s 2 1.0 x 10-2 8.0 x 10-3 2.0 x 10-2 10 mM/s 3 2.0 x 10-2 8.0 x 10-3 2.0 x 10-2 40 mM/s 4 2.0 x 10-2 8.0 x 10-3 1.0 x 10-2 40 mM/s Determine the initial rate of reaction if the initial concentrations of A, B, C are 3 x 10-2 M, 5 x 10-3 M, 5 x 10-5 M, respectively, for the reaction.
Question 9 A rate law for the reaction of HgCl2(aq) with C204- (ag) is expressed as rate equals k left parenthesis Hg CI subscript 2 right parenthesis left parenthesis C subscript 2O subscript 4 to the power of 2 minus end exponent right parenthesis squared (assume the parentheses in the above rate law are brackets) 1. What happens to the rate of the reaction the concentration of HgCl2 is doubled while the concentration of C2044 remains the same? 2. What happens to the rate of the reaction the concentration of C2044 is tripled while the concentration of HgCl2 remains the same? 3. What happens to the rate of the reaction if you double both concentrations of reactants? 4. What is the overall order of the reaction?

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Question 14 Trial # Initial A (M) Initial B (M) Initial Rate (M/s) 1 0.200 0.200 1.20 x 10-3 2 0.200 0.400 2.40 x 10-3 3 0.400 0.200 4.80 x 10-3 Given the table above, use trial #3 to determine k.